Cuprous chloride or copper(I) chloride is a compound with the chemical formula CuCl, consisting of one copper atom and one chlorine atom. It is a white solid with a crystalline structure and is used in various industrial applications, such as as a catalyst and in the production of other copper compounds.
| IUPAC Name | Copper(I) chloride |
| Molecular Formula | CuCl |
| CAS Number | 7758-89-6 |
| Synonyms | Cuprous monochloride, Copper chloride (CuCl), Copper(I) chloride, Cupric chloride, Nantokite |
| InChI | InChI=1S/ClH.Cu/h1H;/q;+1/p-1 |
Copper(I) chloride formula
The formula for Copper(I) chloride is CuCl. This indicates that each molecule of Copper(I) chloride contains one copper atom and one chlorine atom. The formula can be used to calculate the mass of a sample of Copper(I) chloride or the number of moles of Copper(I) chloride present in a sample. The formula also provides information about the relative numbers of atoms present in the compound, which is useful in understanding its properties and behavior.
Copper(I) chloride molar mass
The molar mass of Copper(I) chloride is the mass of one mole of the compound. It is calculated by adding the atomic masses of the elements that make up the compound. Copper(I) chloride has a molar mass of 98.99 g/mol. This value can be used to convert between the mass of a sample of Copper(I) chloride and the number of moles present in the sample.
Copper(I) chloride boiling point
The boiling point of Copper(I) chloride is the temperature at which the compound changes from a liquid to a gas. Copper(I) chloride has a relatively low boiling point of 1,490 °C. This is due to the weak intermolecular forces between the Copper(I) chloride molecules. At this temperature, the molecules gain enough kinetic energy to overcome the attractive forces that hold them together as a liquid.
Copper(I) chloride melting point
The melting point of Copper(I) chloride is the temperature at which the compound changes from a solid to a liquid. Copper(I) chloride has a relatively high melting point of 430 °C. This is due to the strong ionic bonds between the copper and chlorine atoms that make up the compound. At this temperature, the thermal energy supplied to the compound is enough to break the ionic bonds and allow the atoms to move freely as a liquid.
Copper(I) chloride density g/ml
The density of Copper(I) chloride is a measure of its mass per unit volume. Copper(I) chloride has a density of 4.14 g/mL at room temperature. This value indicates that Copper(I) chloride is a dense substance and will sink in liquids that are less dense than it is.
Copper(I) chloride molecular weight
The molecular weight of Copper(I) chloride is the sum of the atomic weights of the atoms in a single molecule of the compound. Copper(I) chloride has a molecular weight of 98.99 g/mol. This value can be used to convert between the mass of a sample of Copper(I) chloride and the number of molecules present in the sample.
Copper(I) chloride Structure
Copper(I) chloride has a crystalline structure in which the copper atoms are surrounded by four chlorine atoms in a tetrahedral arrangement. The copper atoms are bonded to the chlorine atoms by ionic bonds, which result from the transfer of electrons from the copper atoms to the chlorine atoms. This structure gives Copper(I) chloride its characteristic properties, such as its high melting point and density.
| Appearance | White crystalline powder |
| Specific Gravity | 4.14 g/cm³ |
| Color | White |
| Odor | Odorless |
| Molar Mass | 98.99 g/mol |
| Density | 4.14 g/cm³ |
| Melting Point | 430 °C |
| Boiling Point | 1,490 °C |
| Flash Point | Not applicable |
| Water Solubility | 0.0095 g/L at 20 °C |
| Solubility | Soluble in concentrated hydrochloric acid, ammonia, and potassium cyanide. Insoluble in ethanol and ether. |
| Vapour Pressure | Not applicable |
| Vapour Density | Not applicable |
| pKa | Not applicable |
| pH | 4.6 – 5.8 (1% solution) |
Cuprous Chloride Safety and Hazards
Cuprous chloride poses several safety and health hazards. It is harmful if ingested and can cause irritation to the eyes, skin, and respiratory system. Cuprous chloride can also cause metal fume fever, a condition characterized by flu-like symptoms such as fever, chills, and cough. Long-term exposure to Cuprous chloride may cause lung damage and other chronic health effects. When handling Cuprous chloride, it is important to wear protective clothing, gloves, and eye protection to minimize the risk of exposure. In case of accidental ingestion or exposure, seek medical attention immediately. Proper handling, storage, and disposal of Cuprous chloride are necessary to prevent environmental contamination and harm to human health.
| Hazard Symbols | Skull and crossbones |
| Safety Description | Do not ingest. Wear protective clothing, gloves, and eye protection. In case of ingestion or exposure, seek medical attention immediately. Proper handling, storage, and disposal required. |
| UN IDs | UN 3077 |
| HS Code | 28273910 |
| Hazard Class | 6.1 |
| Packing Group | II |
| Toxicity | Toxic if ingested or inhaled. Causes skin and eye irritation. May cause lung damage and other chronic health effects. |
Cuprous Chloride Synthesis Methods
There are several methods to synthesize Cuprous chloride:
One common method involves the reaction between copper and hydrochloric acid. Copper metal reacts with hydrochloric acid to produce CuCl and hydrogen gas. The CuCl can be purified by filtration and drying.
Another method involves the reaction between copper oxide and hydrochloric acid.
To synthesize Cuprous chloride, one can add Copper oxide to a hydrochloric acid solution to produce CuCl2. After that, one can use a reducing agent such as hydrochloric acid or sulfur dioxide to reduce the CuCl2 to form CuCl.
Another method to synthesize CuCl involves dissolving Copper sulfate and Sodium chloride in water, heating the resulting solution, and filtering it to remove impurities. After filtering the resulting solution, it is possible to cool it down to form CuCl crystals.
A variation of this method involves the reaction between copper sulfate and sodium chloride in the presence of reducing agents such as ascorbic acid or glucose. The reducing agent reduces the Cu2+ ions in copper sulfate to Cu+ ions, which then react with the chloride ions in sodium chloride to form CuCl.
Overall, these methods provide a range of options for synthesizing Cuprous chloride, with variations depending on the starting materials and conditions used. Careful attention to safety and environmental considerations is necessary during the synthesis and handling of Cuprous chloride.
Cuprous Chloride Uses
Cuprous chloride has several applications in various fields. Here are some common uses of Cuprous chloride:
- Catalysis: Used as a catalyst in various chemical reactions, including the synthesis of organic compounds such as pharmaceuticals and agrochemicals.
- Pigment: Used as a pigment in ceramics and glass industries. It imparts a green color to the products.
- Antifouling agent: Used as an antifouling agent in marine applications to prevent the growth of barnacles, algae, and other marine organisms on ships and boats.
- Photography: Used as a photographic developer to produce black and white images. It is used as a reducing agent to convert silver ions to metallic silver.
- Electroplating: Used in electroplating to deposit a layer of copper onto a substrate. It is used in the manufacture of electronic components, jewelry, and other products.
- Fungicide: Used as a fungicide to protect plants from fungal diseases.
- Welding: Used in welding to remove oxide layers from metal surfaces before welding.
- Etching: Used as an etching agent in the production of printed circuit boards and other electronic components.
Cuprous chloride finds extensive usage in various industries due to its distinctive properties. Industries use it in diverse applications ranging from catalysis to marine coatings.
Questions:
Q: Is CuCl soluble in water?
A: Yes, CuCl is slightly soluble in water, with a solubility of approximately 0.67 g/L at room temperature.
Q: Is CuCl soluble?
A: CuCl is slightly soluble in water, but insoluble in organic solvents such as ethanol and ether.
Q: What is the name of CuCl?
A: The name of CuCl is Cuprous chloride.
Q: What causes the bubbles when aluminum was placed in solution CuCl? A: When aluminum is placed in a solution of CuCl, a redox reaction occurs, where aluminum reduces the Cu2+ ions in CuCl to Cu+ ions, forming aluminum chloride (AlCl3) and metallic copper (Cu). The bubbles observed are hydrogen gas (H2) produced as a byproduct of the reaction between aluminum and water molecules present in the solution.